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Chemical Kinetics

Chemical kinetics is the study of reaction rates. Learn how to calculate and standardize rates of chemical reactions, plus examples. Explore the concept of progress in reactions and understand concentration measurements affecting reaction rates.

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Chemical Kinetics

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  1. Chemical Kinetics The Study of Reaction Rates

  2. What is a Rate? • The rate of a process in the amount of progress that has been made, divided by the time required to achieve that progress. • Speed = • Example: You travel 102 miles in 2.00 hours • Average Speed = = 51.0

  3. The Rate of a Chemical Reaction • In a chemical reaction, we can define “progress” as the consumption of a reactant or the formation of a product. • To measure this progress, we measure how much a reactant concentration decreases in a given period of time, or how much a product concentration increases in a given period of time.

  4. The Rate of a Chemical Reaction • But not everything in a chemical reaction is changing at the same rate. • 2A(g) + 3B(g)  C(g) + 4D(g) • Suppose the concentration of substance A is decreasing at the rate of 0.40 mol/ L s. What is happening to the other concentrations?

  5. The Rate of a Chemical Reaction • 2A(g) + 3B(g)  C(g) + 4D(g) • = -0.40 • = -0.60 • = 0.20 • = 0.80

  6. Standardizing the Rate of a Chemical Reaction • 2A(g) + 3B(g)  C(g) + 4D(g) • Rate = - = - = = • All of the above expressions give the same result. • - ) = 0.20 • - (-0.60 ) = 0.20

  7. Standardizing the Rate of a Chemical Reaction • 2A(g) + 3B(g)  C(g) + 4D(g) • Rate = - = - = = • Rate = 0.20 • Rate = (0.80 ) = 0.20

  8. Reaction Rate from Concentration Measurements

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